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Nomenclature: Molecular Compounds Most are named by rules of Organic Chemistry Simple Molecular compounds tend to be Binary nonmetallic Use standard prefixes 2 kinds of elements On the Right side of the periodic table

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Nomenclature: Transition Metal Ions Traditional system – –ic ending Considered the most common charge of the ions –ous ending Considered the second most common charge of the ions Based on the trends shown on the periodic table, the most common charge is the highest charge listed; the second most common charges is the lower charge listed.

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Nomenclature: Acid Compounds Binary Acids Contain only hydrogen (H + ) and one other element – a nonmetal These are named with hydro ic acid

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Nomenclature: Acid Compounds Ternary Acids (oxyacids) Contain hydrogen and a polyatomic ion (a oxyradical) that either ends in –ate or –ite. -ate goes to –ic -ite goes to –ous Ponder gum… If you ate it it is icky; but if you bite it, it is delicious.

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Nomenclature: Practice 1. Decide which of the following are expected to be ionic and which are expected to be molecular: a) KF b) N 2 O 5 c) SiCl 4 2. What is the formula of magnesium nitride? 3. What is the formula of calcium phosphate? ionic covalent Mg 3 N 2 Ca 3 (PO 4 ) 2

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Balancing Reactions Based on the Law of Conservation, is present must be preserved. In other words, whatever happens to the reactants must occur to the products. Choose a chemical – insert a coefficient ( multiplier ) in front of it. Never change the subscripts! Treat ions ( radicals ) that appear on both sides as single chunks. ½s can be used for diatomic elements. It is helpful to think of water as HOH, rather than H 2 O.

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Balancing Reactions Whatever happens to the reactants must occur to the products. Choose a chemical – insert a coefficient ( multiplier ) in front of it. Never change the subscripts! Treat ions ( radicals ) that appear on both sides as single chunks. ½s can be used for diatomic elements. It is helpful to think of water as HOH, rather than H 2 O. MgCO 3 + Sn(ClO 3 ) 4 Mg(ClO 3 ) 2 + Sn(CO 3 ) 2 2 1 2 1